Polonium
| |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
| |||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Polonium (symbol: Po) is a chemical element, one of the chalcogens. It is a silvery-white metal with a unique simple cubic structure,[1] although it is rare that polonium or its compounds are encountered in weighable quantities.
Polonium has no stable isotopes, and the metal and all its compounds are intensely radioactive. The power output due to the radioactive decay of polonium-210 is about 140 W g−1, which leads to considerable self-heating and which complicates the investigation of its properties with macroscopic quantities.[1]
Contents
History
Polonium was discovered in 1898 by Marie Curie while she was investigating the radioactivity of pitchblende.[3] The element was named after Curie's native Poland. The discovery earned Marie Curie the Nobel Prize for Chemistry in 1911.[1]
The first weighable quantities of polonium were prepared in 1944 from the lead residues from the Port Hope radium refinery. This polonium had also originally come from uranium ores: it required the treatment of 37 tons of lead dioxide between 1943 and 1945 to produce just 9 mg (40 Ci) of polonium.
Occurrence and production
The only naturally ocurring isotope of polonium is polonium-210 (t½ = 138.38 days), the penultimate member of the radium decay series. It occurs in uranium ores at about 0.1 mg per tonne of ore (a mass fraction of about 10−10). The overall abundance of polonium in crustal rocks can be estimated at about 3 × 10−10 ppm.[1]
Extraction of polonium from natural sources is impractical, and it is produced commercially by the neutron irradiation of bismuth in a nuclear reactor: 20983Bi(n,γ)21083Bi. The bismuth-210 produced undergoes β-decay (t½ = 5.01 days) to give polonium-210.[1] Commercial production is about 85 grams per year, 97% of which is produced by a single facility near Samara in Russia.[4]
Use
Polonium-210 is a vitually pure α-emittor (Eα = 5.30 MeV), with only 0.0011% γ-decay, and is used as an intense source of α-particles.[1]
The main commercial use is in anti-static brushes, which can contain up to 500 µCi (20 MBq) 210Po.[note 2] The α particles ionize molecules from the air, which allows an equalization of charges on the surface being brushed and the helps the mechanical removal of dust particles. Smaller quantities – typically 4–40 kBq (0.1–1.0 µCi) – are occasionally used as α particle sources for teaching and research. In both cases, these are sealed sources.
Polonium-210 is also used in a mixture with beryllium oxide as a portable source of neutrons through the 94Be(α,n)126C reaction. The self-heating of polonium-210 has also been used as a source of heat and/or thermoelectric power in space exploration.[1]
Chemical properties
The chemistry of polonium is similar to that of tellurium, except that the +6 oxidation state is notably less stable due to the inert-pair effect. The principal oxidation states are +2 and +4.
Polonium metal dissolves in dilute acids to give a range of polonium(II) salts. The reaction of polonium with oxygen at 250 °C gives amphoteric polonium(IV) oxide, PoO2, and the the tetrahalides PoCl4 and PoBr4 can also be prepared by the direct reaction of the elements. Polonium(IV) oxide is considerably more basic than its tellurium analogue, and polonium(IV) salts such as the nitrate, sulfate and selenate are known: however, hydrate polonium(IV) oxide, PoO(OH)2, will dissolve in dilute alkali to give salts which are usually written as containing the trioxopolonate(2−) anion, PoO2−3.[1]
Polonium will react with electropositive metals to form polonides. The polonides of the alkali metals and alkaline earth metals can be considered to contain the Po2− anion, and magnesium polonide (MgPo, nickeline structure) will react with dilute acids to give the unstable, gaseous hydrogen polonide, H2Po. The stable polonides of the transition metals and the lanthanoids usually have a 1:1 stoichiometry, and are best considered as intermetallic compunds.[1]
Notes and references
Notes
- ↑ Atomic weight of polonium-210, which is by far the most commonly encountered isotope.
- ↑ Such anti-static brushes (containing less than 500 µCi 210Po) are available in the United States under general domestic licenses: 10 C.F.R. § 31.3 [30 FR 8189, June 26, 1965, as amended at 34 FR 6652, Apr. 18, 1969; 35 FR 3982, Mar. 3, 1970].
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 1.7 1.8 1.9 Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 882–919. ISBN 0-08-022057-6.
- ↑ CRC Handbook of Chemistry and Physics, 62nd ed.; Weast, Robert C., Ed.; CRC Press: Boca Raton, FL, 1981; p E-65. ISBN 0-8493-0462-8.
- ↑ Curie, P.; Curie, M. C. R. Hebd. Acad. Sci. Paris 1898, 127, 175–78.
- ↑ Most Polonium Made Near the Volga River. St. Petersburg Times 2007-01-23, <http://www.sptimesrussia.com/index.php?action_id=2&story_id=20100>.
Further reading
- Polonium; Moyer, Harvey V., Ed.; United States Atomic Energy Commission: Oak Ridge, Tenn., 1956. TID-5221. doi:10.2172/4367751, <http://www.osti.gov/bridge/servlets/purl/4367751-nEJIbm/>.
External links
 |
See also the corresponding article on Wikipedia. |
| Error creating thumbnail: Unable to save thumbnail to destination |
This page is currently licensed under the Creative Commons Attribution 3.0 Unported license and any later versions of that license. |
